4. A constant volume of gas has a pressure of ​98.3 kPa​ at ​497 K​ . Determine the temperature of the gas if the pressure is increased to ​182.5 kPa​ . a) Should the temperature of the gas increase or decrease? b) Using Kinetic Molecular Theory (KMT), explain your answer to (a). ​HINT​: What happens to the particles? c) Determine the final temperature of the gas. P​ 1​= P​ 2​= T​ 1​= T​ 2​= k = k =

they are both synthetic elements

explanation:

d

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

metric time was an attempt to create a standard unit of time based off of 10, but it never took off an is not included in the metric system (si)

answer : (a) volume of the gas = 8.67 ×   l

                (b) second virial coefficient b = -1.21226 l/mole

solution :   given,     t = 300k

                                p = 20atm

                                z = 0.86

                                n = 8.2 mmoles = 8.2 × moles

                                r =   0.082 l atm/k/mol

        find,     (a) volume of gas   and (b) second virial coefficient b at 300k.

formula used :            

                          and            

(a)            

                    = \times 0.082\times 300}{20}[/tex]

                    = 8.67 ×   l

(b)      

                    = (0.00867-1) × 8.659

                    = - 8.5839 l/mole